How long will it take to plate 5.0 g of Ni using a current of 50.0 A and starting with a solution...
Question:
How long will it take to plate 5.0 g of {eq}Ni {/eq} using a current of 50.0 A and starting with a solution of {eq}Ni^{2+} {/eq}?
Electrolysis:
Electrolysis is done to drive the non-spontaneous reduction or oxidation reaction to spontaneity by applying current to the system, thereby supplying electrons. One of the uses of this concept is in electroplating in which a current is passed through a solution of a metal cation and through time, the metal cation is converted to solid metal.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answer
The reduction of nickel(II) ions is:
{eq}Ni^{2+}(aq) +2e^- \to Ni(s) {/eq}
The equation that will be used is:
{eq}m = \dfrac{MIt}{nF} {/eq}
wh...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Electrolysis: Definition, Types & Uses
from
Chapter 20 / Lesson 5
44K
Discover what electrolysis is, how energy changes during an electrolysis reaction, and electrolysis of water and metals. View its manufacturing and industrial uses.
Related to this Question
- How long would it take to electroplate all the Sn4+ in 0.200 L of 0.230 M K2(SnF6) solution with a current of 2.55 A?
- A solution containing Pt4+ is electrolyzed with a current of 4.00 A. How long will it take to plate out all of the platinum in 0.50 L of a 0.010 M solution of Pt4+?
- What current is required to plate out 1.22 g of nickel from a solution of Ni^{2+} in 1.00 hours? (a) 1.11 A (b) 2.22 A
- What current is required to plate out 1.22 g of nickel from a solution of N i 2 + in 0.50 hours?
- A current of 5.34 A is passed through an Sn(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 6.10 grams of tin?
- A current of 4.72 A is passed through a Ni(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 4.90 grams of nickel?
- A current of 5.02 A is passed through a Sn(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 6.30 grams of tin?
- How long will it take to plate out 4.9 kg of Au from aqueous Au3+ with a current of 146.0 A?
- How grams of Ti metal will be deposited from a Ti+4 solution by passing a current of 200 amps for 1 hour?
- A Cr3+(aq) solution is electrolyzed using a current of 6.50 A. a) What mass of Cr(s) is plated out after 3.00 days? b) What amperage is required to plate out 0.280 mol Cr from a Cr3+ solution in a period of 7.70 h?
- A current of 3.84 A is passed through a Sn(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 8.80 g of tin?
- A current of 3.37 A is passed through a Sn(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 9.50 g of tin?
- A current of 3.01 A is passed through a Sn(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 9.00 g of tin?
- A current of 5.41 A is pass through a Ni(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 7.30 g of nickel?
- A current of 4.96 A is passed through a Ni(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 6.80 g of nickel?
- A current of 5.05 A is passed through a Pb(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 6.10 g of lead?
- How many minutes would a solution of Ni^{2+} have to be electrolyzed with a 3.750 A current to plate out 1.94 g of Ni?
- When using a lead-acid battery to start a car, 1.0 g of P b is consumed on the anode. How long will it take to recharge the battery, using a current of .5 amps to turn the P b S O 4 that was produced back into P b ?
- How many minutes would a solution of Fe^{3+} have to be electrolyzed with a 2.130 A current to plate out 2.12 g of Fe?
- A current of 5.61 A is passed through a Ni(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 9.00 g of nickel?
- How many minutes will it take to electroplate 46.1 g of gold by running 5.00 A of current through a solution of
- A current of 3.76 A is passed through a Fe(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 5.70 g of iron?
- A current of 3.65 A is passed through a Fe(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 5.30 g of iron?
- A current of 3.35 A is passed through a Ni(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 4.60 grams of nickel?
- How many minutes would it take to plate out 103 grams of solid nickel from a Ni2+ solution with a current of 2.75 amperes?
- How long would it take to produce 95.0 g of metallic chromium by the electrolytic reduction of Cr3+ with a current of 3.25 A?
- A current of 4.35 A is passed through a Sn(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 5.00 g of tin?
- A current of 4.06 A is passed through a Cu(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 6.50 g of copper?
- A current of 5.25 A is passed through a Pb(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 5.20 g of lead?
- A current of 5.11 A is passed through a C r ( N O 3 ) 2 solution. How long (in hours) would this current have to be applied to plate out 4.50 g of chromium?
- A current of 3.03 A is passed through a Cr(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 6.30 g of chromium?
- How many minutes would it take to plate out 125 grams of solid copper from a Cu2+ solution with a current of 5.35 amperes?
- A Cr3+(aq) solution is electrolyzed using a current of 7.60 A. What mass of Cr(s) is plated out after 2.00 days?
- A current of 4.06 A is passed through a Sn(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 9.30 g of tin?
- How many minutes would a solution of Ni^{2+} have to be electrolyzed with a 3.830 A current to plate out 1.76 g of Ni?
- Calculate the mass of silver deposited when a current of 3 A is passed through a solution of a silver salt for 7 min.
- A current of 3.94 A is pass through a Pb(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 5.40 g of lead?
- How long will it take to electroplate 2.5 pounds Cr on a car bumper using K_2CrO_4 solution and passing 6.0 A current?
- How long would it take to electroplate all the Zn^{2+} in 0.280 L of 0.210 M ZnSO_4 solution with a current of 2.35 A?
- A current of 2.75 amperes is used to electrolyze a solution of copper(II) sulfate. How long will it take to deposit 10.47 grams of copper?
- How long (in minutes), would it take to electroplate all the Au3+ in 0.260 L of 0.220 M [Au(CN)4]Cl solution with a current of 2.50 A?
- A Cr^{3+}(aq) solution is electrolyzed, using a current of 7.60 A. (a) What mass of Cr(s) is plated out after 1.40 days? (b) What amperage is required to plate out 0.200 mol Cr from a Cr^{3+} solution in a period of 8.60 h?
- A current of 341 A is passed through a cr(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 5.30 g of chromium? .....
- A Cr^3+(aq) solution is electrolyzed, using a current of 6.90 A. 1. What mass of Cr (s) is plated out after 1.90 days?
- What mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO_3)_2 solution with a current of 0.500 A for 55.0 s?
- A current of 5.46 A is passed through a Fe(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 6.80 g of iron?
- If we wish to convert 1.00 g of Au3+(aq) ion into Au(s) in a "gold-plating" process, how long must we electrolyze a solution if the current passing through the circuit is 2.00 A?
- Chromium metal can be electroplated from an acidic solution of C r O 3 . What mass of C r , in grams, will be deposited by a current of 98.54 C?
- PLEASE HELP CHEMISTRY HOMEWORK DUE THURSDAY TOMORROW EVENING. KINDLY SHOW ALL WORKINGS AND CALCULATIONS (1). A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be neede
- A current of 5.23 A is passed through a Cr(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 7.50 g of chromium?
- Calculate the potential of the Pb/Pb(IO3)2 electrode in a 0.00466 M solution of NaIO3.
- Calculate the potential of the Pb/Pb(IO3)2 electrode in a 0.00377 M solution of NaIO3.
- Calculate the potential of the Pb/Pb(IO3)2 electrode in a 0.00359 M solution of NaIO3.
- How many minutes will it take to plate out 2.19 grams of chromium metal from a solution of Cr3+ using a current of 35.2 amps in an electrolyte cell?
- How long will it take to plate out each of the following with a current of 100.0 A? a) 1.0 kg Al from aqueous Al^3+ b) 1.0 g Ni from aqueous Ni^2+ c) 5.0 mol Ag from aqueous Ag^+
- A current of 3.50 A is passed through a Sn(NO_3)_2 solution for 1.50 hours. How much tin is plated out of the solution?
- A current of 3.65 A is passed through a Sn(NO3)2 solution for 1.40 hours. How much tin is plated out of the solution?
- A current of 5.74 A is passed through a Sn(NO_3)_2 solution for 1.80 hours. How much tin is plated out of the solution?
- A current of 3.12 A is passed through a Sn(No_3)_2 solution for 1.60 hours. How much tin is plated out of the solution? .............g
- A current of 3.79 A is passed through a Sn(NO3)2 solution for 1.40 hours. How much tin is plated out of the solution?
- In an electroplating experiment, if 2.00 grams of silver was deposited from an AgNO3 solution after passing electric current for 3 hours, what was the current used in amperes?
- What mass of Cu(s) is electroplated by running 20.5 A of current through a Cu2+(aq) solution for 4.00 h?
- What mass of Cu(s) is electroplated by running 26.5 A of current through a Cu2+(aq) solution for 4.00 h?
- A current of 5.50 A is passed through a Sn(NO3)2 solution for 1.80 hours. How much tin is plated out of the solution?
- Calculate the potential of the Pb/Pb(IO_3)_2 electrode in a 0.00840 M solution of NaIO_3.
- How many grams of iron can be produced (plated out) by applying a 3.65 amp current for 87.0 minutes to a solution containing Fe3+ ions? What is the minimum voltage that must be applied for this for this to work? How do you know?
- What mass of Cu(s) is electroplated by running 22.5 A of current through a Cu^2+ (aq) solution for 4.00 h?
- Calculate G (maximum electrical work obtainable) when 7.10 g of C l 2 ( g ) are consumed in the reaction C d ( s ) + C l 2 ( g ) C d 2 + ( a q ) + 2 C l ( a q ) , E c e l l = 1.76 V . (a) 3.40 10 6 J (b) 3.40 10 4 J (c) 1.70
- What current is required to plate (1.50 x 10^0) g of copper from a copper(II) nitrate solution in (5.500 x 10^0) hours?
- How long will it take to plate out each of the following with a current of 107.1 A? (a) 6.7 kg Al from aqueous Al^3+. (b) 6.7 g Ni from aqueous Ni^2+. (c) 8.3 mol Ag from aqueous Ag^+.
- A C r 3 + ( a q ) solution is electrolyzed, using a current of 7.50 A. What mass of C r ( s ) is plated out after 1.80 days? What amperage is required to plate out 0.300 mol C r ( s ) from a C r 3 + solution in a period of 7.20 h?
- What mass of silver is deposited when current of 2.6 A is passed through a solution of silver salt for 40 minutes?
- Calculate the potential of the Pb/Pb(IO_3)_2 electrodes in a 0.00824 M solution of NaIO_3.
- A current of 3.36 A is passed through a Fe(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 6.50 g of iron?
- Calculate the potential of a silver electrode in contact with the following: a. solution that is 0.0150 M in I2 and saturated with AgI b. solution that is 0.0040 M in CN- and 0.0600 M in Ag(CN)2^-.
- Calculate the potential of a silver electrode in contact with the following: (a) A solution that is 0.0150 M in I_2 and saturated with AgI. (b) A solution that is 0.0040 M in CN^- and 0.0600 M in
- How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgNO3 solution using a current of 20 amps?
- How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgNO_3 solution using a current of 30 amps?
- 0.222 g of a divalent metal is deposited when a current of 0.45 A is passed through a solution of it's salt for 25 min using appropriate electrodes. Calculate the relative atomic mass of the metal. (1 Faraday = 96500 c/mol)
- What is the current necessary to plate out 5.0 g of copper metal in 2.0 hours from a copper (ii) nitrate solution?
- An electrolysis cell is operated for 3000 s using a current of 1.50 A. From which 1.0 m solution will the greatest mass of metal be deposited?
- a current of 4.21 A is passed through a Ni(NO3)2 solution for 1.40 hours how much nickel is plated out of the solution in grams?
- How many grams of iron metal will be deposited from a solution that contains Fe2+ ions if a current of 1.08 A is applied for 56.1 minutes?
- How many grams of iron metal will be deposited from a solution that contains Fe2+ ions if a current of 1.05 A is applied for 58.6 minutes?
- Calculate the amount of silver deposited at cathode when 5 ampere of current is passed for 50 minutes through a solution of Ag NO_3.
- A current of 3.77 A is passed through an Sn(NO3)2 solution for 1.40 hours. How much tin is plated out of the solution?
- A current of 3.03 A is passed through a Cu(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 7.10 g of copper?
- How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO_4 for 90.0 min?
- Calculate E_o , E, and ?G for the following cell reactions (a) Mg(s) + Sn^2+(aq) ? Mg^2+(aq) + Sn(s) where [Mg2+] = 0.055 M and [Sn^2+] = 0.030 M E_o = V E = V ?G = kJ (b) 3Zn(s) + 2Cr^3+(aq) ? 3Zn^2+
- How many seconds will be required to produce 1.0 g of chromium metal by the electrolysis of a Cr(NO_3)_3 solution using a current of 3.0 A? a. 3.6 x 101 b. 6.3 x 102 c. 9.7 x 102 d. 1.9 x 103 e. 3
- How many seconds will be required to produce 1.0 g of chromium metal by the electrolysis of a Cr(NO_3)3 solution using a current of 3.0 A? a. 3.6\times10^1 b. 6.3\times10^2 c. 9.7\times10^2 d. 1.9\tim
- How many seconds would it take to deposit 0.500 g of Ni metal on an electrode by passing a 3.00 amp current through a solution of Ni^{2+}?
- How long must a current of 5.00 amperes be applied to a solution of silver ions to produce 10.5 grams of silver?
- How many minutes will it take to plate out 4.50 g of Cu from a solution of Cu(NO3)2 (aq) onto the cathode of an electrolytic cell when 8.00 A of current are used? 1. 28.5 min 2. 3.06 x 10^-9 min 3
- Calculate E 0 , E , and ? G for the following cell reactions: (a) Mg(s) + Sn^{2+} (aq) \rightleftharpoons Mg^2+(aq) + Sn(s) where [ M g 2 + ] = 0.045 M and [ s n 2 + ] ? 0.055 M (b). 3 Z a (
- A current of 5.62 A is passed through a Fe(NO_3)_2 solution for 1.50 hours. How much iron is plated out of the solution? ..... g
- A current of 4.91 A is passed through a Fe(NO_3)_2 solution for 1.40 hours. How much iron is plated out of the solution?
- A current of 3.05 A is passed through a Fe(NO3)2 solution for 1.50 hours. How much iron is plated out of the solution?
- A current of 3.65 A is passed through a Fe(NO3)2 solution for 1.20 hours. How much iron is plated out of the solution?
- A current of 3.41 A is passed through a Cr(NO_3)_2 solution. How long (in hours) would this current have to be applied to plate out 5.30 g of chromium? .................h
Explore our homework questions and answers library
Browse
by subject